600 cc of a gas at a pressure of 750 mm is compressed to 500 cc. Taking the temperature to remain constant, the increase in pressure is                                           

(a) 150 mm                       (b) 250 mm

(c) 350 mm                       (d) 450 mm

An ideal gas expands according to PV=constant. On expansion, the temperature of gas:

(1) will rise

(2) will drop

(3) will remain constant

(4) cannot be determined because the external pressure is not known

The compressibility of a gas is less than unity at STP. Therefore:

(1) V_m > 22.4 litre                           

(2) V_m < 22.4 litre

(3) V_m = 22.4 litre                           

(4) V_m = 44.8 litre

The numerical value of C_p-C_v for one mole of the ideal gas is equal to:

1. R             

2. R/M

3. M/R         

4. None of the above

In which case is the rate of diffusion highest if all are present in the same container at the same temperature:

1. 4 g H₂

2. 32 g O₂

3. 22 g CO₂

4. 56 g N₂

Partial pressure of Hydrogen in Flask containing 2 gm of H₂ and 32 gm of SO₂ is 

1. 1/16 of total pressure

2. 1/2 of total pressure

3. 2/3 of total pressure

4. 1/8 of total pressure

At high pressure, the compressibility factor 'Z' is equal to -

1.  Unity

$2.$ $1-\frac{\mathrm{Pb}}{\mathrm{RT}}$
$3.$ $1+\frac{\mathrm{Pb}}{\mathrm{RT}}$

4.  Zero

The density of O₂(g) is maximum at:-

1. STP

2. 273 K and 2 atm 

3. 546 K and 1 atm

4. 546 K and 2 atm

A gas diffuses four time quickly as oxygen. The molecular weight of gas is:

1. 2

2. 4

3. 8

4. 16

If density of vapours of a substance of molar mass 18 gm / mole at 1 atm pressure and 500 K is 0.36 kg m^–3 , then value of Z for the vapours is : (Take R = 0.082 L atm mole K^–1)

(1) $\frac{41}{50}$

(2) $\frac{50}{41}$

(3) 1.1

(4) 0.9